Question: calculate pH of 50.0 mL acetate buffer + 1.00 mL 0.6 M NaOH Moles  CH3COOH OH- CH3COO-  before addition  ? ? ? Addition  ? ? ? after addition  ? ? ?       (below is the data to answer the answer)    Deionized water Acetate Buffer Ammonia Buffer    pH of solution 6.62 4.59 9.49   Ph of solution after addition of 1 mL  of 0.6 M NaOH 12.41 4.71 9.50   pH of solution after addition of 1 mL of 0.6 M HCl  1.38 3.87 9.24                       Preparation of Buffer solutions  Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00

Which of the following will produce a buffer solution?     Question options:   mixing 100 mL of 0.1 M hydrofluoric acid and 100 mL of 0.1 M HCl   mixing 100 mL of 0.1 M HCl and 100 mL of 0.1 M sodium fluoride   mixing 50 mL of 0.1 M HCl and 100 mL of 0.1 M sodium fluoride

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Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)